Zn + H2SO4 = ZnSO4 + H2O Given that ; Sample = 4.01 g H2 = 0.0932 g Molar mass o

Question

Zn + H2SO4 = ZnSO4 + H2O

Given that ;

Sample = 4.01 g

H2 = 0.0932 g

Molar mass of H 2 = 2.016 g/ mole

Number of moles = amount in g / molar mass

= 0.0932 g/ 2.016 g/ mole

= 0.046 mole H2

Now calculate the mole s of Zn as follows:

0.046 mole H2* 1 mole Zn /1 mole H2 = 0.046 mole Zn

Amount of Zn in sample = number of moles * molar mass of Zn

= 0.046 mole Zn *65.3800 g/mol

=3.023 g

Percentage purity of Zn = amount of Zn in g/ sample amount in g ]*100

= 3.023 g /4.01 g]*100

= 75.37 %

In the given sample there is 75.37 % pure Zn rest of impurity.

Explanation / Answer

I got this wrong can someone help answer it correctly

3. An impure sample of zinc (Zn) is treated with an excess of sulfuric acid (H,SO,) to form zinc sulfate ZnSO4) and molecular hydrogen (H2 a. Write a balanced equation for the reaction. puit3 b. I10.0932 g of H2 is obtained from 4.01 g of the sample, calculate the percent purity of the sample @y tic What assumptions must you make in (b)? c. (o

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